Acid Base Intro (AP Chem)

Match each of the following acids to its conjugate base

• HPO₄^-2

• H₂SO₄

• HSO₄^-

• H₂PO₄^-

• SO₄^-2

• HSO₄^-

• H₂PO₄^-

• H₃PO₄

• PO₄^-3

• HPO₄^-2

In the following reaction, NH₃ is a Bronsted-Lowry ______.

NH₃ + H₂O → NH₄⁺ + OH^-

• acid

• base

• conjugate acid

• conjugate base

Organize these acids and bases into the right categories

Groups:

(a) strong acid

,

(b) strong base

,

(c) weak acid

,

(d) weak base

• KOH

• HNO₂

• HI

• NH₄OH

• Fe(OH)₂

• HNO₃

• H₃PO₃

In the reaction:

HCO₃^1– + H₂O ↔ CO₃^2– + H₃O⁺

the hydrogen carbonate ion (HCO₃^1–) is acting as a ___.

• acid

• base

• indicator

• conjugate

Identify the acids involved in the equilibrium reaction:

CN^– + H₂O ↔ HCN + OH^–

• CN^– and H₂O

• H₂O and HCN

• CN^– and OH^–

• H₂O and OH^–

Which of the following represents a conjugate acid-base pair?

• SO₃^2– : SO₂

• CO₃^2– : CO₂

• H₃O⁺ : H₂

• NH₄⁺ : NH₃

Arrhenius acids __________.

• dissociate to make H⁺ ions in solution

• dissociate to make OH^- ions in solution

• are proton acceptors

• have pH values higher than 7

Bronsted-Lowry bases ___________.

• dissociate to make H⁺ ions in solution

• dissociate to make OH^- ions in solution

• are H⁺ donors

• are H⁺ acceptors

Which of the following products would result from NH₃ acting as a bronsted base when reacting with water:

NH₃ + H₂O --> ____________

• NH₄ + OH

• NH₄⁺ + OH^-_

• NH₂ + H₃O

• NH₂^- + H₃O⁺

An Arrhenius base:

• donates H+

• accepts H+

• produces H+

• produces OH-